Question

37)Into a 15.00-liter container at 25°C are placed 1.00 moles of O2 gas and 3.00 moles of solid C (graphite). If the carbon and oxygen react completely to form CO(g), what will be the final pressure in the container at 25°C? a) 0.274 atm b) 1.00 atm c) 4.89 atm d) 1.63 atm e) 3.26 atm

39) N2 (g) + 3H2 (g) 2NH3 (g). If a 3.4 L flask is first charged with 1.2 atm of nitrogen, then hydrogen is added until the total pressure reaches 4.0 atm, what is the maximum pressure of ammonia that can be produced at a constant 50 o C? a) 1.2 atm b) 1.9 atm c) 2.4 atm d) 2.7 atm e) 3.6 atm

Answer 1

37)
2 C(s) + O2 (g) —> 2 CO(g)

mol of CO formed = 2*mol of O2
= 2*1.00 mol
= 2.00 mol

Initially there were 1 mol of gas but now there are 2 mol of gas

So, pressure will double

Lets find the initial pressure of gas:
Given:
V = 15.0 L
n = 1.00 mol (this is initial mol of gas)
T = 25.0 oC
= (25.0+273) K
= 298 K

use:
P * V = n*R*T
P * 15 L = 1 mol* 0.08205 atm.L/mol.K * 298 K
P = 1.630 atm

So,
final number of mol of gas = 2*1.630 atm
= 3.26 atm

Answer: e

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